Cleaning Up With Atom Economy

ACETONE INTRODUCTION Acetone, is a colorless, highly volatile and flammable liquid with a distinct acrid odour. Acetone is the simplest yet most important ketone. Even though it is considered a chemical, it can also be found in our body in low- levels from the breakdown of fat and it can be used by our body in normal processes like making sugar and fat. It is a polar organic solvent that has various industrial uses like being a solvent in varnishes, lacquers, paints, printing inks and photographic films. PRODUCTION PROCESS The Catalytic Dehydrogenation of Isopropanol Catalysts Involved: Solid copper, Iron, or Nickel Conversion of Isopropanol: 87.8% Process of Manufacturing: 1) Isopropanol is heated using steam in order to be vaporized. 2) It is then compressed to a reactor pressure of 4-5 atms. 3) It enters a catalytic shell with a tulbular catalytic reactor, which is lined with a catalyst. The reactor operates at 400-500°C using flue glass for heating. 4) The flue gas passes in the shell side of the shell and tube reactor. 5) A reaction occurs. 6) The gasses are condensed using a cooling water dispenser. 7) The condensed isopropanol and acetone are sent for acetone fractionation.

Acetone Fractionation Column 1) There will be byproducts in the form of hydrogen gas, diisopropyl ether, and propylene. 2) Hydrogen gas will be removed using a water scrubber. The added water will ensure the solubility of the acetone and isopropanol. 3) Acetone will be cleaved from isopropanol and water. 4) The isopropanol and water will be sent to a isopropanol column. Isopropanol Column 1) Water will be produced as the bottom product and isopropanol as the top product. 2) Water will be recycled, since it cannot be divided from the product completely. 3) Water is cooled using a water condenser and will be sent to the water scrubber as fresh water solvent.

ATOM ECONOMY ANALYSIS The synthesis of BPA is than using acetone in the presence of acetone and phenol formulate using the desired product, As the desired product of BPA then you can substitute the values of product and equation. Although consideration of both, the atom economy and the percent yield gives a much better measure of the efficiency of a reaction of acetone and its environmental acceptability to the other factor need to be considered. The percentage of atom economy of Acetone this can be done by taking the ratio of the mass of the utilized atoms(137 of the total mass of the atoms of all reactants (275 and multiplying by 100 as shown below this reaction has the only 50percent of atom economy then calculated by 100 percent is equal to 5.808percent or 13.68percent of atom economy of Acetone. ECONOMIC IMPORTANCE Acetone, also known as 2-propanone or dimethyl ketone (DMK), is an important chemical intermediate used in the production of acrylic plastics, polycarbonates, and epoxy resins. These materials in turn are used by many different industry sectors to produce countless everyday items. Due to the ongoing pandemic, the industrial use of acetone has gradually diminished making its use limited. However, it can still be of use because it can be used to sterilize medical tools and medical equipment that are needed these days.

IMPLICATIONS Acetone is not harmful to humans, other living organisms and environment when used properly. Acetone is safe in normal amounts but can be dangerous when not used in proper way. It is extremely flammable which is why it is not recommended to be used when near a fire source. Acetone can also be found in nature not just in chemical products that are commonly used at home. Excess exposure to acetone can cause skin irritation, cough, headache, dizziness, unconsciousness, nose irritation, eye irritation and lung irritation. These are the reasons why one should store this chemical properly. To store acetone properly make sure to keep it inside of a container away from children’s reach and far from fire and electrical source. VI. References: MEMBERS: Cite the sources in APA format Matias, Ella I.C.I.S. (2010, April 23). Acetone Production and Manufacturing Robosa, May Ann Process. Retrieved October 08, Serrano, Cyril Villamor, Alyza 2020, from Tiopes, Kyle https://www.icis.com/explore/resources/news/2007/11/01/9074860/ac etone-productionand-manufacturing-process/ Chemical Engineering Guy. (2019, February 5). Acetone Production Scheme - Petrochemical Process (Lec086) [Video]. YouTube. https://www.youtube.com/watch? v=-bozu62FvYA Rai, Anand. [Anand Rai]. (2018). Preparation of Phenol from cumene (Cumene process) [Video]. YouTube. https://www.youtube.com/watch?v=YF3hW0PtNmc Yong, Yap Wei. [Yap Wei Yong]. (2018, June 01). PETROCHEMICAL PROCESSES - PRODUCTION OF ACETONE (A149243) [Video]. YouTube. https://www.youtube.com/watch?v=s__aQt-gMAc Zelman, K.J., MPH, RD, LD (2019, August 19). WebMD Medical References. from https://www.webmd.com/diet/what-is-acetone Acetone: The Hidden Hazard. (2019, August 22). Retrieved October 10, 2020, from https://www.msdsonline.com/2013/06/18/acetone-the-hidden-hazard/

SSooddiiuumm FFlluuoorriiddee By Group 3 - 11 STA Samantha Jonota, Julliane Manuzon, What is Sodium Fluoride? Jessica Quejada, Ian Relox, Ralph Tamani What is Sodium Fluoride? Sodium Fluoride (NaF) is an inorganic salt made of municipal water fluoridation system that is best known for its vital role in preventing dental caries. It may be added to toothpastes or mouthwashes or to municipal water supplies for this purpose. Sodium Fluoride is a colorless crystalline solid that dissolves into liquid or a white powder. It is soluble in water and can be used to fluorinate supplies as a wood preservative, in cleaning compounds, manufacture of glass, and many other uses. Sodium fluoride is noncombustible and corrosive to aluminum. Fluorine (F) is the most reactive chemical element and the lightest member of the halogen elements of the periodic table. It binds calcium ions in the hydroxyapatite of surface tooth enamel, preventing corrosion of tooth enamel by acids. This agent may also inhibit acid production by commensal oral bacteria. Sodium (Na) is the most common alkali metal and the sixth most abundant element on Earth. It is a necessary constituent of plant and animal tissue. Ingesting too much fluoride causes gastrointestinal problems, however in toothpaste, there are only small amounts that are very low to really cause detrimental effects. By introducing fluoride to saliva, it enables the teeth to take in the fluoride. It then interacts with calcium and phosphate to form Fluorapatite. Fluorapatite is what makes the teeth stronger and more resistant to cavity. pg. 1

PRODUCTION PROCESS: Sodium Fluoride is present in salt and fresh water, it is Next, Sodium Fluoride is also found in mining as formed through neutralization which is when an acid the rare mineral Villiaumite which is found in and a base form a salt and water The salt made from the North and South America and some parts of reaction will have equal weights of the acid and base, Africa and Europe. Lastly, it is also a byproduct The neutralization of a strong acid ad weak base will made when phosphate fertilizers are being made. have a pH of less than 7, and conversely, the resulting Apatite (a form of calcium phosphate that pH when a strong base neutralizes a weak acid will be contains Fluoride) is crushed and treated with greater than 7. It is called neutralization when salts that Sulfuric Acid (H2SO4). This reaction also are formed from neutralization reactions have produces Phosphoric Acid (H3PO4), Calcium equivalent concentrations of weights of acids and Sulfate (CaSO4), Hydrogen Fluoride (HF), and bases. Hydrogen Fluoride (HF) is neutralized by Sodium Silicon Tetrafluoride (SiF4). The hydrogen fluoride Hydroxide (NaOH) giving us Sodium Fluoride (NaF) and and silicon tetrafluoride can then be converted Water (H2O), it comes in a form of powder. into sodium fluoride by treating it with sodium carbonate (Na2CO3) Atom Economy Analysis: Preparation: Industrial production is the major source of sodium fluoride. It is commonly prepared by Neutralizing Hydrofluoric Acid with bases such as Sodium with bases such as sodium carbonate (soda ash, Na2CO3), Sodium Hydroxide (caustic soda, NaOH) or sodium bicarbonate (NaHCO3). Hydrogen Fluoride (HF) is neutralized by Sodium Hydroxide (NaOH) giving us Sodium Fluoride (NaF) and Water (H2O), it comes in a form of powder. HF + NaOH NaF + H2O H= 1+1= 2 H= 2 F= 1 F= 1 Na= 1 Na= 1 O= 1 O=1 A.E = (mass of useful product/ mass of all products) x 100 pg. 2

SOLUTION: pg. 3 Hydrofluoric Atom Economy = (mass of useful Acid (HF) H= 1 x 1 = 1g F= 1 x 19 = 19g product / = 1g + 19g mass of all products) x 100 = 20 g/mol = [ (42g/mol) / (120g/mol) ] x 100 SodiumHydroxide (NaOH) Na= 1 x 23 = 23g OH= 1 x 17 = 17g = 0.35 x 100 = 23g + 17g = 35% = 40 g/mol Sodium Flouride (NaF) The Atom Economy of producing Na= 1 x 23 = 23g F= 1 x 19 = 19g Sodium Flouride is 35% = 23g + 19g = 42 g/mol aipstoTramohndeceiupnhccereoeofmnAfctioheniccmisaisaeslynylt.hyistnpaiwsesw:aaohyfilctoohwit Water (H2O) H= 1 x 2 = 2g O= 1 x16 = 16g = 2g + 16g = 18 g/mol HF +NaOH NaF + H2O (20g/mol) + (40g/mol) (42g/mol) + (18g/mol) →(Na2CO3): 2HF + Na2CO3 Sodium fluoride occurs naturally as the mineral villiaumite, 2NaF + H2O + CO2 although the compound is not produced commercially from that source. Some sodium fluoride is obtained as a byproduct of the manufacture of phosphate fertilizers. In that process, apatite (a form of calcium phosphate that also contains fluorides and/or chlorides) is crushed and treated with sulfuric acid (H2SO4). The products of that reaction include phosphoric acid (H3PO4), calcium sulfate (CaSO4), hydrogen fluoride (HF), and silicon tetrafluoride (SiF4). The hydrogen fluoride and silicon tetrafluoride can then be converted into sodium fluoride. The compound can also be produced by treating hydrogen fluoride with sodium carbonate

Economic Importance pg. 4 ShocotoapfsaorfwdscraPhnotepoiohwarutasrnobhoimmoseddepdmcdnpuuacoutufoFcscoomcloltttmtruteespispmistod.nrpuoLeruaroduaiSsalnduenabenoFdentedorgdeDodvx,riicdifaAenpusliitrgeuemtsionraasrficstnedmyroaFoocsibr.nenulom.adugfngmslTioetbfspehfpraxe,edeiegoidrsbeueeouutlsnninefsscutdoteiaistscdndhbk.hetFiaihAnlasaotialdtssrsytittaseothosasaet It isn't just for these, it can also be used in a different angle and useful industries such as continuous casting powder raw materials in the steel industry, in water treatment, disinfectants, and pesticides in agriculture, for disinfecting fermentation apparatus in breweries and distilleries, ceramic pigments, metal plating, surface coatings, foundry additives for aluminum foundry, cover flux, filler for bonded abrasives in metallurgical industry and as raw materials to make chemical fluoride in enamel industry, industry-feed making, construction materials and many more. IMPLICATION Sodium Fluoride is a very useful compound, but it has its restrictions. It has a dangerous level rate of 6.1. Its hazard classification and labelling are in danger according to harmonized classification and labelling (CLP00) approved by the European Union. The exposure routes possible are inhalation, ingestion, skin, and/or eye contact. Meanwhile, animals eating food grown in the contaminated soil take on this additional burden of fluoride pollution from the environment. Sodium Fluoride can also be dangerous to plants by its exposure to fluoride accumulates in the foliage of plants and mainly occurs through the atmosphere or root absorption of soil.

Proper ways to properly store Sodium Fluoride is under the shade that pg. 5 has ventilation. These are important because its melting point is at 993 ℃ its boiling point is at 1695 ℃ and its relative density is at 2.558. Usage and intake of dosage are based on your age and the fluoride content in your water supply. When the atom economy decreases its percentage, the production of the desired product which is sodium fluoride will decrease as well. A lot of manufacturers and their economic usage will decrease and can be negatively affected. When it increases, it will give good effects that will help humans in their everyday lifestyle stated at the economic importance part. The byproduct or excess product during the production of sodium fluoride is H2OuaatSosagFolcwoarspdrmloowAuodwigaivafcstin(noeehiitrnahtatuhueuenTvoteroeesnspi.lensmyaahieng.ttrtrdtaeanvandushee.aae,sdvWsuwitndcrsegrstlmaeswFoielioraeeiehaeitrell.pwnndessslauieilchooIpsacnaemtodnoetdapnlureodcmntniitreiveregkhr,sorhsivdtcoteedahtaneioasoaehiinmrucessnnittspnaeeolnfteisnbidudeoietthstidgscrilsnuasdrhhonctme,ooitaggyftseuaesttoapfaatmiteoahsrretidmrrcwnlooncoaelriooeoieetfddlnuweiianmlrtrassslssuie.nsfpnleedftis.acans,Ilaetsorapcialttooecavnnnrtsagreratshpaaainrdiayaeeruodctnteltpindrtdmstigfuripdsyviodisoienhvunatmuetwe.ernoenelioslalstenioWataoaeugeuptdtxtnotniufudhgfnhpmeacteifafeasnssteiioeqterSltdsee.esgeurrcuoyoeersberntrststIpado,scushmtysoaalttiouiicnemlgsauikeiooieoinnso(ietsnemenntnnsegoin.tyde.tetoeomgssts,eo..)h,,yd)de water.

pg. 6 CITATIONS: National Center for Biotechnology Information (2020). PubChem Compound Summary for CID 5235, Sodium fluoride. Retrieved October 7, 2020 from https://pubchem.ncbi.nlm.nih.gov/compound/Sodium-fluoride. Libretexts. (2020, August 15). Neutralization. Retrieved October 07, 2020 from https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Suppleme ntal_Modules_(Physical_and_Theoretical_Chemistry)/Acids_and_Bases/Acid//Base_Reactions/Neutraliza tion Sodium fluoride Formula - Sodium Fluoride Uses,Properties, Structure and Formula. (n.d.). Retrieved October 09, 2020 from https://softschools.com/formulas/chemistry/sodium_fluoride_uses_properties_structure_formula/301/ Xinbo (2020, September 16). Sodium fluoride Formula - Sodium Fluoride Uses, Properties, Structure and Formula. (n.d.). Retrieved October 09, 2020 from https://softschools.com/formulas/chemistry/sodium_fluoride_uses_properties_structure_formula/301/ Xinbo (2020, September 16).Sodium Fluoride Industrial Grade, Retrieved from October 07, 2020 from Zhuzhou Xinbo Chemical Co.,Ltd.:https://xinbo-chem.com/product/sodium-fluoride-industrial-grade/ U.S. Department of Health & Human Services, U. (2019, October 30). CDC - NIOSH Pocket Guide to Chemical Hazards - Sodium fluoride (as F). Retrieved October 08, 2020 from https://www.cdc.gov/niosh/npg/npgd0563.html Group 3 Grade 11 St. Teresa of Avila Submitted to: Ms. Angela May Mendoza Louise Samantha Jonota – Introduction and Layout & Design Ian Harvey Relox Julliane Erycka Manuzon -Production Process – Implication & Revisions Ralph Tamani Jessica Nadine Quejada -Economic Importance -Atom Economy Analysis









I.INTRODUCTION Copper sulfate or Cupric Sulfate (CuSO4) is a combination of copper and sulfur. It is an inorganic compound that can kill bacteria, algae, roots, plants, snails, and fungi. Its color ranges from grayish white in powder from to blue color in the form of crystal. Copper Sulfate is commonly used in cosmetics, drugs, and as a food additive, however, it can be toxic to humans and the environment depending on the copper content. II. PRODUCTION PROCESS Copper sulfate can be made through the process of neutralization reaction. In neutralization reaction, the acid and base react to form water and salt. When a solution is neutralized, salts are formed from equal weights of acid and base. Copper (II) hydroxide and sulfuric acid when mixed in equimolar amounts would form copper sulfate. When you allow the solution to evaporate without heating, it would produce a bright blue copper (II) sulfate pentahydrate crystals (CuSO4·5H2O). If sulfate pentahydrate is heated strongly, the hydration waters would drive off and it would result in a fine white powder or anhydrous copper (II) sulfate (CuSO4).

III. Atom Economy Analysis: Finding the Atom Economy of producing copper sulphate CuO + H₂SO₄ -> CuSO₄ + H₂O Finding the A.E = molecular mass of the desired product/molecular mass of all reactants x 100 Molecular mass of CuO = 37 Molecular mass of H₂SO₄ = 50 Molecular mass of CuSO₄ = 77 (77 / [37 + 50]) x 100 (77 / 87) x 100 0.885 x 100 88.5% The atom economy of producing copper sulfate is 88.5% CuO + H₂SO₄ -> CuSO₄ + H₂O The atom economy of producing copper sulfate by reacting cupric oxide and sulfuric is 88.5% This process has a high atom economy and is therefore an efficient way to make copper sulfate. It uses minimal resources (using only 1 piece of cupric oxide and sulfuric acid) and produces only 1 by-product being water which can be profitable to whoever will make copper sulfate using this reaction. This reaction since it has a high atom economy makes little waste materials that have to be disposed of since the materials are renewable and the by product can be used elsewhere. In conclusion this reaction, even though it doesn’t have a 100% atom economy is a very efficient way to make copper sulfate since its atom economy is 88.5%, its reactants are renewable, and its only by product is water which is useful elsewhere

IV. ECONOMIC IMPORTANCE Copper Sulfate has a big role, help and importance in our society. Some products containing copper sulfate can be used in organic agriculture such as fertilizer, pest control, and water treatments. Agricultural applications is one of the most common uses of Copper Sulfate, having numerous functions throughout the care and management of crops. It is often used as a fertilizer, increasing the copper content of the soil. This can help to correct peaty and acidic soils in order to create a hospitable climate for plant growth. And it can also be used to address mildew, leaf spots, blight and apple scabs on field fruit trees, nut trees, and vegetables. Copper sulfate is used as a drying agent in the anhydrous form, as an additive for fertilizers and foods, and several industrial applications such as textiles, leather, wood, batteries, ink, petroleum, paint, and metal, among others. It is also used as an animal nutritional supplement. Copper sulfate is a versatile, flexible, and effective compound perfect in countless applications given it’s different uses in different kinds of ways and forms.

V.IMPLICATIONS Based on the U.S. EPA, they considered that copper sulfate to be moderately toxic by ingestion. The higher the volume of copper sulfate that is exposed, the higher the chances of experiencing side effects such as nausea and vomiting (High exposure may lead to worse injuries) Humans may be exposed to copper in drinking water. Volunteers consumed copper filtered water at concentrations ranging from 0-12 mg / L. There were reports of nausea beginning at 4 mg / L and vomiting at 6 mg / L. We can see here that as the volume ingested increases, the more solutions containing copper sulfate raised the mass for nausea and vomiting. Avoid high exposure. Scientists measured the total copper ion in human blood serum after ingesting copper sulfate. Mean blood copper levels of 287 µg / L Cu were correlated with moderate toxicity and 798 µg / L Cu were correlated with serious toxicity. Due to the harmful effects of Copper sulfate, it should be properly stored in a tightly sealed container. When using Copper sulfate, a person must avoid repeated exposure when handling the product. Safety glasses, chemical- resistant gloves, lab coat, and respiratory equipment shall be worn. Always read and follow the label of a product, especially when applying pesticides containing copper sulfate. Products containing copper sulfate have signal words that range from caution to danger. The signal word refers to the combined toxicity of the active and other ingredients in the product. A sudden increase in the manufacturing of Copper sulfate, may be helpful especially to those who regularly use it. However, the usage of it may be abused due to the huge amount being processed. On the other hand, a sudden decrease in the manufacturing of Copper sulfate may affect particularly those who utilize it for agricultural purposes.

Significance of Copper Sulfate. (2017). World of Chemicals. Retrieved from https:// www.worldofchemicals.com/578/chemistry- articles/significance-of- coppersulfate.html#:~:text=Copper%20sulfate%20is%20use d%20in,vital%20role%20in%20painting%20glas ses. National Center for Biotechnology Information (2020). PubChem Compound Summary for CID 24462, Copper sulfate. Retrieved October 8, 2020 from https://pubchem.ncbi.nlm.nih.gov/compound/Coppersulfate. Boone, C., Gervais, J., Luukinen, B., Buhl, K., & Stone, D., (2012). Copper Sulfate Technical Fact Sheet. National Pesticide Information Center, Oregon State University Extension Services. Retrieved from http://npic.orst.edu/factsheets/archive/cuso4tech.html. ChemAlert (2016). Copper sulfate. Retrieved from https://www.nyrstar.com/~/media/Files/N/Nyrstar/ sustainability/safety-data-sheets-australia- english/Nyrstar%20Hobart%20- %20Copper%20Sulphate.pdf. Applications: Copper Compounds - Copper Sulphate. (2019). Retrieved from Copper.org website: https://www.copper.org/resources/properties/compounds/ copper_sulfate01.html Copper Sulfate Technical Fact Sheet. (n.d.). Retrieved from npic.orst.edu website: http:// npic.orst.edu/factsheets/archive/cuso4tech.html#:~:text=Co pper%20sulfate%20is%20used%20as

Jessie Olaño - Introduction and References Christine Relevo - Economic Importance and Layout artist Sophia Sombrano - Production Process and Implications Christopher Ventosa - Computation and Analysis Gabriel Verzosa - Implications